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Ch.3 - Mass Relationships in Chemical Reactions
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145당신이 사용하는 게 아니라요?교과서 변경
모든 교과서McMurry 8th EditionCh.3 - Mass Relationships in Chemical Reactions문제 73a
3장, 문제 73a

Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen: N2H4 + O2 → N2 + 2 H2O (a) How many grams of O2 are needed to react with 50.0 g of N2H4?

검증된 단계별 안내
1
Determine the molar mass of N_2H_4 by adding the atomic masses of nitrogen and hydrogen.
Calculate the number of moles of N_2H_4 using the given mass (50.0 g) and its molar mass.
Use the balanced chemical equation to find the mole ratio between N_2H_4 and O_2.
Calculate the number of moles of O_2 needed using the mole ratio from the balanced equation.
Determine the mass of O_2 required by multiplying the moles of O_2 by its molar mass.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
2m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to calculate how much of each substance is needed or produced based on balanced chemical equations. In this case, understanding the stoichiometric coefficients from the reaction equation is essential to determine the amount of O2 required for the reaction with a given mass of N2H4.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. For this problem, calculating the molar mass of N2H4 and O2 will enable the conversion of grams to moles, facilitating the determination of the required amount of O2.
추천 영상:
가이드 코스
02:11
Molar Mass Concept

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It ensures the law of conservation of mass is upheld. In this scenario, the balanced equation N2H4 + O2 → N2 + 2 H2O provides the necessary ratios of reactants and products, which are essential for calculating the amount of O2 needed to react with a specific mass of N2H4.
추천 영상:
가이드 코스
01:32
Balancing Chemical Equations
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교과서 질문

Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen: N2H4 + O2 → N2 + 2 H2O (b) How many grams of N2 are obtained if the yield is 85.5%?

1310
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